LEAD - Pb - [plumbum]

Gray with a bluish shade, heavy, very soft, malleable, plastic metal. Low-melting, on air becomes covered by a steady oxidic film. Possesses small reactionary ability. It is passivated in water, hydrochloric acid, the diluted sulfuric acid, the concentrated nitric acid. Doesn't react with hydrate of ammonia. Weak reducer. Transferred to solution by the concentrated sulfuric acid, diluted nitric acid. Is oxidized by oxygen, halogens, chalcogens.


Molar mass g/mol 207.2
Density g/cm3 11.337
Melting point °C 327.502
Boiling point °C 1745

Methods for the preparation of Lead:

Pb(NO3)2 + Zn = Pb↓ + Zn(NO3)2.

Pb(NO3)2 + 2H2O → Electrolysis → Pb↓(on cathode) + O2↑(on anode) + 2HNO3.

PbSO4(damp) + Zn(plate) = Pb↓(sponge) + ZnSO4.

PbCl2 + H2 = Pb + 2HCl (300-350°C).

PbS + H2 = Pb + H2S (400-600°C).

PbS + 2PbO = 3Pb + SO2 (800-900°C).


Сhemical reactions with Lead:

Pb + 3H2SO4(conc.>80%) = Pb(HSO4)2 + SO2↑ + 2H2O (30-50°C).

Pb + 2H2SO4(conc.) = PbSO4↓ + SO2↑ + 2H2O (boiling).

3Pb + 8HNO3(diluted, hot) = 3Pb(NO3)2 + 2NO↑ + 4H2O.

Pb + 2NaOH(conc.) + 2H2O = Na2[Pb(OH)4] + H2↑.

2Pb + O2 = 2PbO (over 600°C).

3Pb + 2O2 = (Pb2IIPbIV)O4 (400-500°C).

Pb + E2 = PbE2 (200-300°C, E = F, Cl, Br, I).

Pb + 2F2 = PbF4 (400-500°C).

Pb + 2HF = PbF2 + H2 (160°C).

Pb + E = PbE (800-1200°C, E = S, Se, Te).

2Pb(powder) + 2H2O + O2 = 2Pb(OH)2↓ (time).

2Pb + H2O + O2 + CO2 = Pb2CO3(OH)2↓ (time).


 

Did you know?

The only two non-silvery metals are gold and copper.